An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am

An element cannot be broken down to other substances by chemical reactions

-

A compound consists of two or more elements in a fixed ratio- e.g. Sodium (Na, element, metal); chlorine (Cl, element, poisonous gas); NaCl (compound, edible table salt)

-

Elements change characteristics when in the form of compounds-

Elements and Compounds

H, C, N, O (99% of elements in the human body)-Na, Mg, P, S, Cl, K, Ca (0.9%)-F, V, Cr, Mn, Fe, Co, Cu, Zn, Mo, Se, I, (Trace elements)-Ni, B, Si (unknown)-

Elements essential for life

Element deficiency

Basis of life-Makes complex molecules possible-Basis of Dna, carbohydrates and lipids-=< 4 covalent bonds-Can have functional groups substitutes for hydrogen atoms, allowing for diversity

-

Carbon

Hydrocarbons are stores of fuel (fat/adipose, petrol)-

Some H atoms in carbon skeletons (R) can be replaced-Functional groups contribute to molecular diversity

Comparison of male and female sex hormones

Both are based of the four closed ring cholesterol group differing only in two functional groups

Oxygen: 2 bonds-Nitrogen: 3 bonds-Carbon: 4 bonds-Bond angles are defined and cannot change (e.g. water will always be a v shaped molecule with a bonding angle of 120o

-

Defined 3D structure determined by bond angles and lengths-Oxygen - red; Nitrogen - blue; Carbon - black (grey); Hydrogen - white-

Covalent bonds have defined geometries

1800: opiates relieve pain and have world altering effects on the brain (hallucinations)

-

Why does the brain have receptors to something not made by the body-1975: Discovered that endorphins made by pituitary were a response to pain and stress

-

Molecular shape determines function

Because the shape of morphine is similar to that of a natural endorphin, morphine combines to those receptors and alleviates pain.

-

The Aqueous Environment- Polar nature of water

-

Weak interactions- Non-covalent interactions

-

Weak interactions in an aqueous environment are essential for biological functions

Water is a polar molecule as there are opposite charges as either end of the molecule

-

Hydrogen has a partial positive charge while oxygen has a partial negative, meaning that the top end of the molecule (oxygen) is negative while the bottom end (hydrogen) is positive

-

Water is a polar molecule

Weaker than covalent bonds-Easily broken by random thermal motion-Continuously formed and broken-Can form bonds with 4 other water molecules-

Hydrogen bonds

Solid state of water is more dense than liquid (ice is 10% less dense than water - why it floats)

-

When ice warms up (thermal energy) lattice structures melt and the water molecules become closer to each other

-

Water's polarity attracts it to ionic and polar molecules-Very good at dissolving bonds-Hydrophilic means water loving-Hydrophobic means water fearing-Water forms a hydration shell around ionic groups-Dissolves compounds by forming hydrogen bonds-Negative charge of oxygen forms a bond with the positive charge of sodium. Because of the large amount of water molecules, these can form a shell around individual sodium molecules

-

The same occurs with chlorine and hydrogen-

Water molecules

Hydrogen must be attached to an electronegative atom (e.g. oxygen or nitrogen)

-

Hydrogen bonding properties of water are due to being polar-Strongest when three atoms in a line-DNA double helix: base pairing-Protein folding: alpha-helix, beta-sheet-

Hydrogen bonds

Non-covalent interactions make cellular processes-Most interactions in biology are short lived - weak, specific and reversible-Ligand and receptor interaction, respond, separate e.g. signalling between cells

-

DNA replication: need to separate the two DNA strands of double helix-Proteins fold into the correct shapes but need to move and breathe allowing it to alter structure and bind to something else

-

Peptide passing through a pore in a cell membrane (if bonded, it would be bound permanently to amino acids)

-

Advantages of weak bonds

Many biomolecules are polar- Proteins- DNA- Carbohydrates

-

Dissolved in water-Can interact via non-covalent interactions e.g. Hydrogen bonding-Proteins can bring together through complimentary charges-If there are many complimentary charges, it will be tightly bound-If there are few complimentary charges, the bond will be weak-Individual hydrogen bonds are very weak however if there are many bonds, they become quite strong

-

Shape and structure determines function-Specificity-Interaction of varied strengths possible-

Interaction of biomolecules in the aqueous environment of the cell

Subunits can form covalent bonds to form macromolecules-Macromolecules can use non-covalent bonds (mostly hydrogen) to form macromolecular assemblies

-

E.g.: Sugars, amino acids and nucleotides form covalent bonds to create globular proteins and RNA which form non-covalent bonds to form ribosomes

-

Non-covalent bonds involved with protein synthesis

Molecular DiversityTuesday, 10 March 2015 9:34 am